Bonding: Shapes of molecules

                     Linear 

• 2 electron pairs = 2 bonding pairs/0 lone pairs
• Bond angle = 180 degrees
• E.g. BeCl2           

Trigonal planar

• 3 electron pairs = 3 bonding pairs/0 lone pairs
• Bond angle = 120 degrees
• E.g. BF3

Tetrahedral

• 4 electron pairs = 4 bonding pairs/0 lone pairs
• Bond angle = 109.5 degrees
• E.g. CH4

Trigonal pyramidal

• 4 electron pairs = 3 bonding pairs/1 lone pair
• Bond angle = 107 degrees
• E.g. NH3

Bent (v-shape)

• 4 electron pairs = 2 bonding pairs/2 lone pairs
• Bond angle = 104.5 degrees
• E.g. H20

Trigonal bipyramidal

• 5 electron pairs = 5 bonding pairs/0 lone pairs
• Bond angle = 90/120 degrees
• E.g. PF5

Trigonal pyramidal/see-saw

• 5 electron pairs = 4 bonding pairs/ 1 lone pair
• Bond angle = 119/89 degrees
• E.g. SF4

Trigonal planar/ T-shape

• 5 electron pairs = 3 bonding pairs/2 lone pairs
• Bond angle = 89 degrees
• E.g. ICl3

Octahedral

• 6 electron pairs = 6 bonding pairs/0 lone pairs
• Bond angle = 90 degrees
• E.g. SF6

Square planar

• 6 electron pairs = 4 bonding pairs/2 lone pairs
• Bond angle = 90 degrees
• E.g. XeF4

Square pyramid

• 6 electron pairs = 5 bonding pairs/1 lone pair
• Bond angle = 89 degrees
• E.g. IF5